chemistry data booklet

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Data Booklet

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7 6 5 4 3 2

1 8 9

Table of Common Polyatomic Ions

acetate (ethanoate) ammonium benzoate borate carbide carbonate hydrogen carbonate perchlorate chlorate chlorite hypochlorite chromate dichromate cyanide hydroxide iodate nitrate nitrite oxalate hydrogen oxalate permanganate peroxide persulfide phosphate hydrogen phosphate dihydrogen phosphate silicate sulfate hydrogen sulfate sulfite hydrogen sulfite hydrogen sulfide thiocyanate thiosulfate CH₃COO –

NH₄+

C₆H₅COO –

BO₃3 – C₂2 –

CO₃2 – HCO₃–

CIO₄– CIO₃–

CIO₂– OCl – _{or CIO} –

Cr O₄2 –

Cr₂O₇2 –

CN –

OH – IO₃–

NO₃– NO₂–

OOCCOO2 – HOOCCOO–

MnO₄– O₂2 –

S₂2 –

PO₄3 –

HPO₄2 – H₂PO₄–

SiO₃2 – SO₄2 –

HSO₄– SO₃2 –

HSO₃– HS –

SCN – S₂O₃2 – hydrogen

1 1.01

2.2

1+,1–

lithium

3 6.94

Li

H

1.0

1+

sodium

11

22.99

Na

0.9

1+

potassium

19 39.10

K

0.8

1+

rubidium

37 85.47

Rb

0.8

1+

cesium

55 132.91

Cs

0.8

1+

francium

87 (223)

Fr

0.7

1+

radium

88 (226)

Ra

0.9

2+

barium

56 137.33

Ba

0.9

2+

strontium

38 87.62

Sr

1.0

2+

calcium

20 40.08

Ca

1.0

2+

scandium

21 44.96

Sc

1.4

3+

titanium

22 47.87

Ti

1.5

4+, 3+

zirconium

40 91.22

Zr

1.3

4+

niobium

41 92.91

Nb

1.6

5+, 3+

vanadium

23 50.94

V

1.6

5+, 4+

chromium

24 52.00

Cr

1.7

3+, 2+

hafnium

72 178.49

Hf

1.3

4+

tantalum

73

180.95

Ta

1.5

5+

tungsten

74 183.84

W

1.7

6+

rhenium

75 186.21

Re

1.9

7+

osmium

76 190.23

Os

2.2

4+

ruthenium

44 101.07

Ru

2.2

3+

iron

26

55.85

Fe

1.8

3+, 2+

cobalt

27 58.93

Co

1.9

2+, 3+

rhodium

45 102.91

Rh

2.3

3+

iridium

77 192.22

Ir

2.2

4+

technetium

43 (98)

Tc

2.1

7+

manganese

25 54.94

Mn

1.6

2+, 4+

molybdenum

42 95.94

Mo

2.2

6+

rutherfordium

104 (261)

Rf

dubnium

105 (262)

Db

seaborgium

Sg

bohrium

107 (264)

106 (266)

Bh

hassium

108

(277)

Hs

meitnerium

109 (268)

Mt

yttrium

39 88.91

Y

1.2

3+

magnesium

12 24.31

Mg

1.3

2+

beryllium

4 9.01

Be

1.6

2+

lanthanum

57 138.91

La

1.1

3+

cerium

58

140.12

Ce

1.1

3+

praseodymium

59

140.91

Pr

1.1

3+

neodymium

60

144.24

Nd

1.1

3+

samarium

62

150.36

Sm

1.2

3+, 2+

promethium

61 (145)

Pm

—

3+

actinium

89 (227)

Ac

1.1

3+ 4+

thorium

90

232.04

Th

1.3

4+

protactinium

91 231.04

Pa

1.5

5+, 4+

uranium

92 238.03

U

1.7

6+, 4+

plutonium

94 (244)

Pu

1.3

4+, 6+

neptunium

93 (237)

Np

1.3

5+ References

Lide, D.R. 2005. CRC Handbook of Chemistry and Physics. 86th_{ed. Boca Raton: CRC Press.}

Speight, James G. 2005. Lange’s Handbook of Chemistry. 16th_{ed. New York: McGraw-Hill, Inc.}

IUPAC commission on atomic weights and isotopic abundances. 2002. http://www.chem. qmw.ac.uk/iupac/AtWt/index.html.

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18 17 16 15 14 13 12 11 10

Note: The legend denotes the physical state of the elements at exactly 101.325 kPa and 298.15 K.

Legend for Elements

Most stable ion charges

Name

Atomic molar mass (g/mol)*

Symbol Electronegativity Atomic number

Key

iron

26

55.85

Fe

1.8

3+, 2+

europium

63

151.96

Eu

—

3+, 2+

americium

95

(243)

Am

—

3+, 4+

gadolinium

64

157.25

Gd

1.2

3+

curium

96

(247)

Cm

—

3+

terbium

65

158.93

Tb

—

3+

berkelium

97

(247)

Bk

—

3+, 4+

dysprosium

66

162.50

Dy

1.2

3+

californium

98

(251)

Cf

—

3+

holmium

67

164.93

Ho

1.2

3+

einsteinium

99

(252)

Es

—

3+

erbium

68

167.26

Er

1.2

3+

fermium

100

(257)

Fm

—

3+

thulium

69

168.93

Tm

1.3

3+

mendelevium

101

(258)

Md

—

2+, 3+

ytterbium

70

173.04

Yb

—

3+, 2+

nobelium

102

(259)

No

—

2+, 3+

lutetium

71

174.97

Lu

1.0

3+

lawrencium

103

(262)

Lr

—

3+

aluminium

13

26.98

Al

1.6

3+

boron

5

10.81

B

2.0

silicon

14

28.09

Si

1.9

carbon

6

12.01

C

2.6

arsenic

33

74.92

As

2.2

—

phosphorus

15

30.97

P

2.2

—

nitrogen

7

14.01 3.0

—

selenium

34

78.96

Se

2.6

—

sulfur

16

32.07

S

2.6

—

oxygen

8

16.00 3.4

—

tellurium

52

127.60

Te

2.1

—

bromine

35

79.90

Br

3.0

—

chlorine

17

35.45 3.2

—

fluorine

9

19.00 4.0

—

iodine

53

126.90

I

2.7

—

astatine

85

(210)

At

2.2

—

krypton

36

83.80 —

argon

18

39.95 —

neon

10

20.18 —

helium

2

4.00 —

xenon

54

131.29 2.6

radon

86

(222) —

gallium

31

69.72

Ga

1.8

3+

indium

49

114.82

In

1.8

3+

thallium

81

204.38

Tl

1.8

1+, 3+

germanium

32

72.64

Ge

2.0

4+

tin

50

118.71

Sn

2.0

4+, 2+

lead

82

207.2*

* The isotopic mix of naturally occurring lead is more variable than other elements, preventing precision to greater than tenths of a gram per mole.

Pb

1.8

2+, 4+

antimony

51

121.76

Sb

2.1

3+, 5+

bismuth

83

208.98

Bi

902 254 1.9 3+, 5+ polonium

84

(209)

Po

2.0 2+, 4+ zinc

30

65.41

Zn

1.7

2+

cadmium

48

112.41

Cd

1.7

2+

mercury

80

200.59

Hg

1.9

2+, 1+

copper

29

63.55

Cu

1.9

2+, 1+

silver

47

107.87

Ag

1.9

1+

gold

79

196.97

Au

2.4

3+, 1+

nickel

28

58.69

Ni

1.9

2+, 3+

palladium

46

106.42

Pd

2.2

2+, 3+

platinum

78

195.08

Pt

— — — — 2.2 4+, 2+ roentgenium

111

(272)

Rg

darmstadtium

110

(271)

Ds

— — — — — — — — —

He

Ne

Ar

Cl

F

O

N

Kr

Xe

Rn

* Based on C

( ) Indicates mass of the most stable isotope

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Chemistry Notation

Symbol Term Unit(s)

c specific heat capacity J/(g

.

°C) or J/(g

.

K)

E° standard electrical potential V or J/C

E_k kinetic energy kJ

E_p potential energy kJ

∆H enthalpy (heat) kJ

∆_fH° standard molar enthalpy of formation kJ/mol

I current A or C/s

K_c equilibrium constant —

K_a acid ionization (dissociation) constant —

K_b base ionization (dissociation) constant —

M molar mass g/mol

m mass g

n amount of substance mol

P pressure kPa

Q charge C

T temperature (absolute) K

t temperature (Celsius) °C

t time s

V volume L

c amount concentration mol/L

Symbol Term

∆ delta (change in)

° standard

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Miscellaneous

25.00 °C is equivalent to 298.15 K

Specific Heat Capacities at 298.15 K and 100.000 kPa

c_air = 1.01 J/(g

.

°C)

c_{polystyrene foam cup} = 1.01 J/(g

.

°C) c_copper = 0.385 J/(g

.

°C)

c_aluminium = 0.897 J/(g

.

°C)

c_iron = 0.449 J/(g

.

°C)

c_tin = 0.227 J/(g

.

°C)

c_water = 4.19 J/(g

.

°C)

Water Autoionization Constant (Dissociation Constant)

K_w = 1.0 × 10–14 at 298.15 K (for ion concentrations in mol/L)

Faraday Constant

F = 9.65 × 104 C/mol e–

Quadratic Formula

x

a

b b ac

2 4

2

!

= -

-Selected SI Prefixes

Prefix Exponential Symbol Value

tera T 1012

giga G 109

mega M 106

kilo k 103

milli m 10–3

micro µ 10–6

nano n 10–9

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Standard Molar Enthalpies of Formation at 298.15 K

Name Formula ∆_fH° (kJ/mol)

aluminium oxide Al₂O₃(s) –1 675.7

ammonia NH₃(g) –45.9

ammonium chloride NH₄Cl(s) –314.4

ammonium nitrate NH₄NO₃(s) –365.6

barium carbonate BaCO₃(s) –1 213.0

barium chloride BaCl₂(s) –855.0

barium hydroxide Ba(OH)₂(s) –944.7

barium oxide BaO(s) –548.0

barium sulfate BaSO₄(s) –1 473.2

benzene C₆H₆(l) +49.1

butane C₄H₁₀(g) –125.7

calcium carbonate CaCO₃(s) –1 207.6

calcium chloride CaCl₂(s) –795.4

calcium hydroxide Ca(OH)₂(s) –985.2

calcium oxide CaO(s) –634.9

calcium sulfate CaSO₄(s) –1 434.5

carbon dioxide CO₂(g) –393.5

carbon monoxide CO(g) –110.5

chromium(III) oxide Cr₂O₃(s) –1 139.7

copper(I) oxide Cu₂O(s) –168.6

copper(II) oxide CuO(s) –157.3

copper(II) sulfate CuSO₄(s) –771.4

copper(I) sulfide Cu₂S(s) –79.5

copper(II) sulfide CuS(s) –53.1

dinitrogen tetroxide N₂O₄(g) +11.1

ethane C₂H₆(g) –84.0

ethanoic acid (acetic acid) CH₃COOH(l) –484.3

ethanol C₂H₅OH(l) –277.6

ethene (ethylene) C₂H₄(g) +52.4

ethyne (acetylene) C₂H₂(g) +227.4

glucose C₆H₁₂O₆(s) –1 273.3

hydrogen bromide HBr(g) –36.3

hydrogen chloride HCl(g) –92.3

hydrogen fluoride HF(g) –273.3

hydrogen iodide HI(g) +26.5

hydrogen perchlorate HClO₄(l) –40.6

hydrogen peroxide H₂O₂(l) –187.8

hydrogen sulfide H₂S(g) –20.6

iron(II) oxide FeO(s) –272.0

iron(III) oxide Fe₂O₃(s) –824.2

iron(II,III) oxide (magnetite) Fe₃O₄(s) –1 118.4

lead(II) bromide PbBr₂(s) –278.7

lead(II) chloride PbCl₂(s) –359.4

lead(II) oxide (red) PbO(s) –219.0

lead(IV) oxide PbO₂(s) –277.4

magnesium carbonate MgCO₃(s) –1 095.8

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Standard Molar Enthalpies of Formation at 298.15 K

cont’d

Name Formula ∆_fH° (kJ/mol)

magnesium hydroxide Mg(OH)₂(s) – 924.5

magnesium oxide MgO(s) – 601.6

magnesium sulfate MgSO₄(s) – 1 284.9

manganese(II) oxide MnO(s) – 385.2

manganese(IV) oxide MnO₂(s) – 520.0

mercury(II) oxide (red) HgO(s) – 90.8

mercury(II) sulfide (red) HgS(s) – 58.2

methanal (formaldehyde) CH₂O(g) – 108.6

methane CH₄(g) – 74.6

methanoic acid (formic acid) HCOOH(l) – 425.0

methanol CH₃OH(l) – 239.2

nickel(II) oxide NiO(s) – 240.6

nitric acid HNO₃(l) – 174.1

nitrogen dioxide NO₂(g) + 33.2

nitrogen monoxide NO(g) + 91.3

octane C₈H₁₈(l) – 250.1

pentane C₅H₁₂(l) – 173.5

phosphorus pentachloride PCl₅(s) – 443.5

phosphorus trichloride (liquid) PCl₃(l) – 319.7

phosphorus trichloride (vapour) PCl₃(g) – 287.0

potassium bromide KBr(s) – 393.8

potassium chlorate KClO₃(s) – 397.7

potassium chloride KCl(s) – 436.5

potassium hydroxide KOH(s) – 424.6

propane C₃H₈(g) – 103.8

silicon dioxide (α-quartz) SiO₂(s) – 910.7

silver bromide AgBr(s) – 100.4

silver chloride AgCl(s) – 127.0

silver iodide AgI(s) – 61.8

sodium bromide NaBr(s) – 361.1

sodium chloride NaCl(s) – 411.2

sodium hydroxide NaOH(s) – 425.8

sodium iodide NaI(s) – 287.8

sucrose C₁₂H₂₂O₁₁(s) – 2 226.1

sulfur dioxide SO₂(g) – 296.8

sulfuric acid H₂SO₄(l) – 814.0

sulfur trioxide (liquid) SO₃(l) – 441.0

sulfur trioxide (vapour) SO₃(g) – 395.7

tin(II) chloride SnCl₂(s) – 325.1

tin(IV) chloride SnCl₄(l) – 511.3

tin(II) oxide SnO(s) – 280.7

tin(IV) oxide SnO₂(s) – 577.6

water (liquid) H₂O(l) – 285.8

water (vapour) H₂O(g) – 241.8

zinc oxide ZnO(s) – 350.5

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Solubility of Some Common Ionic Compounds in Water at 298.15 K

Ion

Group 1 ions NH₄+ NO₃– ClO₃– ClO₄– CH₃COO–

F–

Cl– Br–

I–

SO₄2–

CO₃2– PO₄3– SO₃2–

IO₃–

OOCCOO2– OH

–

Solubility greater than or equal to 0.1 mol/L

(very soluble)

most most most most

Group 1 ions Group 1 ions Group 1 ions

NH₄+

NH₄+ Co(IO₃)₂

Fe₂(OOCCOO)₃

NH₄+

Solubility less than 0.1 mol/L

(slightly soluble)

RbClO₄

CsClO₄

AgCH₃COO

Hg₂(CH₃COO)₂ Li+

Mg2+

Ca2+ Sr2+ Ba2+ Fe2+ Hg₂2+

Pb2+

Cu+ Ag+ Hg₂2+

Pb2+ Tl+

Ca2+ Sr2+ Ba2+ Ag+ Hg₂2+

Pb2+ Ra2+

most most most

Note: This solubility table is only a guideline that is established using the K_sp values. A concentration of 0.1 mol/L

corresponds to approximately 10 g/L to 30 g/L depending on molar mass. Hg₂2+ is a polyatomic ion of mercury.

Flame Colour of Elements

Element Symbol Colour lithium Li red

sodium Na yellow

potassium K violet

rubidium Rb violet

cesium Cs violet

calcium Ca yellowish red

strontium Sr scarlet red

barium Ba yellowish green

copper Cu blue to green

boron B yellowish green

lead Pb blue-white

Note: The flame test can be used to determine the identity of a metal or a metal ion. Blue to green indicates a range of

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Table of Selected Standard Electrode Potentials*

Reduction Half-Reaction Electrical Potential E° (V)

F2(g) + 2 e– ⇌ 2 F–(aq)...+2.87

PbO2(s) + SO42–(aq) + 4 H+(aq) + 2 e– ⇌ PbSO4(s) + 2 H2O(l) ...+1.69

MnO4–(aq) + 8 H+(aq) + 5 e– ⇌ Mn2+(aq) + 4 H2O(l) ...+1.51

Au3+(aq) + 3 e– _⇌ Au(s) ...+1.50

ClO₄–(aq) + 8 H+(aq) + 8 e– _⇌ Cl–(aq) + 4 H₂O(l) ...+1.39

Cl2(g) + 2 e– ⇌ 2 Cl–(aq) ...+1.36

2 HNO2(aq) + 4 H+(aq) + 4 e– ⇌ N2O(g) + 3 H2O(l) ...+1.30

Cr₂O₇2–(aq) + 14 H+(aq) + 6 e– _⇌ 2 Cr3+(aq) + 7 H₂O(l) ...+1.23

O₂(g) + 4 H+(aq) + 4 e– _⇌ 2 H₂O(l) ...+1.23

MnO2(s) + 4 H+(aq) + 2 e– ⇌ Mn2+(aq) + 2 H2O(l) ...+1.22

Br2(l) + 2 e– ⇌ 2 Br–(aq) ...+1.07

Hg2+(aq) + 2 e– _⇌ Hg(l) ...+0.85

OCl–(aq) + H₂O(l) + 2 e– _⇌ Cl–(aq) + 2 OH–(aq) ...+0.84

2 NO3–(aq) + 4 H+(aq) + 2 e– ⇌ N2O4(g) + 2 H2O(l) ...+0.80

Ag+(aq) + e– _⇌ Ag(s) ...+0.80

Fe3+(aq) + e– _⇌ Fe2+(aq) ...+0.77

O₂(g) + 2 H+(aq) + 2 e– _⇌ H₂O₂(l) ...+0.70

I2(s) + 2 e– ⇌ 2 I–(aq) ...+0.54

O2(g) + 2 H2O(l) + 4 e– ⇌ 4 OH–(aq) ...+0.40

Cu2+(aq) + 2 e– _⇌ Cu(s) ...+0.34

SO₄2–(aq) + 4 H+(aq) + 2 e– _⇌ H₂SO₃(aq) + H₂O(l) ...+0.17

Sn4+(aq) + 2 e– _⇌ Sn2+(aq) ...+0.15

S(s) + 2 H+(aq) + 2 e– _⇌ H2S(aq) ...+0.14

AgBr(s) + e– _⇌ Ag(s) + Br–(aq) ...+0.07

2 H+(aq) + 2 e– _⇌ H₂(g) ... 0.00

Pb2+(aq) + 2 e– _⇌ Pb(s) ...– 0.13

Sn2+(aq) + 2 e– _⇌ Sn(s) ...– 0.14

AgI(s) + e– _⇌ Ag(s) + I–(aq) ...– 0.15

Ni2+(aq) + 2 e– _⇌ Ni(s) ...– 0.26

Co2+(aq) + 2 e– _⇌ Co(s) ...– 0.28

PbSO4(s) + 2 e– ⇌ Pb(s) + SO42–(aq) ...– 0.36

Se(s) + 2 H+(aq) + 2 e– _⇌ H₂Se(aq) ...– 0.40

Cd2+(aq) + 2 e– _⇌ Cd(s) ...– 0.40

Cr3+(aq) + e– _⇌ Cr2+(aq) ...– 0.41

Fe2+(aq) + 2 e– _⇌ Fe(s) ...– 0.45

NO₂–(aq) + H₂O(l) + e– _⇌ NO(g) + 2 OH–(aq) ...– 0.46

Ag₂S(s) + 2 e– _⇌ 2 Ag(s) + S2–(aq) ...– 0.69

Zn2+(aq) + 2 e– _⇌ Zn(s) ...– 0.76

2 H2O(l) + 2 e– ⇌ H2(g) + 2OH–(aq) ...– 0.83

Cr2+(aq) + 2 e– _⇌ Cr(s) ...– 0.91

Se(s) + 2 e– _⇌ Se2–(aq) ...– 0.92

SO42–(aq) + H2O(l) + 2 e– ⇌ SO32–(aq) + 2OH–(aq) ...– 0.93

Al3+(aq) + 3 e– _⇌ Al(s) ...–1.66

Mg2+(aq) + 2 e– _⇌ Mg(s) ...–2.37

Na+(aq) + e– _⇌ Na(s) ...–2.71

Ca2+(aq) + 2 e– _⇌ Ca(s) ...–2.87

Ba2+(aq) + 2 e– _⇌ Ba(s) ...–2.91

K+(aq) + e– _⇌ K(s) ...–2.93 Li+(aq) + e– _⇌ Li(s) ...–3.04

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R

el

at

iv

e S

tr

en

gt

hs o

f A

ci

ds a

nd B

as

es a

t 2

98 .1

5 K

C om m on N am e IU PA

C / S

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be nzo ic a ci d be nz en ec ar bo xy lic a ci d C6 H5 C O O H (a q) C6 H5 CO O – (a q) 6. 3 × 1 0 –5 ac et ic a ci d et ha no ic a ci d CH 3 C O O H (a q) CH 3 CO O – (a q) 1. 8 × 1 0 –5 di hy dr og en c itr at e i on C3 H5 O (C O O H )2 CO O – (a q) C3 H5 O CO O H (CO O )2 2– (a q) 1.7 × 1 0 –5 bu ta no ic a ci d C3 H7 C O O H (a q) C3 H7 CO O – (a q) 1. 5 × 1 0 –5 pr op an oi c a ci d C2 H5 C O O H (a q) C2 H5 CO O – (a q) 1. 3 × 1 0 –5 ca rb on ic a ci d ( C O2 + H 2 O) aq ue ou s h yd ro ge n c ar bo na te H2 CO 3 (a q) HC O3 – (a q) 4. 5 × 1 0 –7 hy dr og en c itr at e i on C3 H5 O CO O H (CO O )2 2– (a q) C3 H5 O (C O O)3 3– (a q) 4. 0 × 1 0 –7 hy dr os ul fu ri c a ci d aq ue ou s h yd ro ge n s ul fid e H2 S( aq ) HS – (a q) 8.9 × 1 0 –8 hy dr og en s ul fit e i on H SO 3 – (a q) SO 3 2– (a q) 6. 3 × 1 0 –8 di hy dr og en p ho sp ha te i on H2 PO 4 – (a q) H PO 4 2– (a q) 6. 2 × 1 0 –8 hy po ch lo ro us a ci d aq ue ou s h yd ro ge n h yp oc hl or ite H O Cl (a q) O Cl – (a q) 4. 0 × 1 0 –8 hy dr oc ya ni c a ci d aq ue ou s h yd ro ge n c ya ni de H C N (a q) CN – (a q) 6. 2 × 1 0 – 10 am m on iu m i on NH 4 + (a q) NH 3 (a q) 5. 6 × 1 0 – 10 hy dr og en c ar bo na te i on HC O3 – (a q) CO 3 2– (a q) 4.7 × 1 0 – 11 hy dr og en a sc or ba te i on HC 6 H6 O6 – (a q) C6 H6 O6 2– (a q) 2. 0 × 1 0 – 12 hy dr og en p ho sp ha te i on H PO 4 2– (a q) PO 4 3– (a q) 4. 8 × 1 0 – 13 wa te r H2 O (l) OH – (a q) 1. 0 × 1 0 – 14 N ot e: A n a pp ro xi m at io n m ay b e u se d i ns te ad o f t he q ua dr at ic f or m ul a w he n t he c on ce nt ra tio n o f H 3 O

+ p

ro du ce d i s l es s t ha n 5 % o f t he o ri gi na l a ci d co nc en tr at io n ( or t he c on ce nt ra tio n o f t he a ci d i s 1 0 00 t im es g re at er t ha n t he Ka

). A

n a pp ro xi m at io n c an a ls o b e u se d f or w ea k b as es

. T

he f or m ul as of t he c ar bo xy lic a ci ds h av e b ee n w ri tt en s o t ha t t he C O O H g ro up c an b e e as ily re co gn iz ed

. E

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Acid–Base Indicators at 298.15 K

Indicator AbbreviationsSuggested pH Range Colour Change as pH Increases K_a

methyl violet HMv(aq) / Mv–(aq) 0.0 – 1.6 yellow to blue ~2 × 10–1

cresol red H2Cr(aq) / HCr

–_(aq)

HCr–(aq) / Cr2–(aq)

0.0 – 1.0 7.0 – 8.8

red to yellow yellow to red

~3 × 10–1 3.5 × 10–9

thymol blue H2Tb(aq) / HTb

–_(aq)

HTb–(aq) / Tb2–(aq)

1.2 – 2.8 8.0 – 9.6

red to yellow yellow to blue

2.2 × 10–2 6.3 × 10–10

orange IV HOr(aq) / Or–(aq) 1.4 – 2.8 red to yellow ~1 × 10–2

methyl orange HMo(aq) / Mo–(aq) 3.2 – 4.4 red to yellow 3.5 × 10–4

bromocresol green HBg(aq) / Bg–(aq) 3.8 – 5.4 yellow to blue 1.3 × 10–5

methyl red HMr(aq) / Mr–(aq) 4.8 – 6.0 red to yellow 1.0 × 10–5

chlorophenol red HCh(aq) / Ch–(aq) 5.2 – 6.8 yellow to red 5.6 × 10–7

bromothymol blue HBb(aq) / Bb–(aq) 6.0 – 7.6 yellow to blue 5.0 × 10–8

phenol red HPr(aq) / Pr–(aq) 6.6 – 8.0 yellow to red 1.0 × 10–8

phenolphthalein HPh(aq) / Ph–(aq) 8.2 – 10.0 colourless to pink 3.2 × 10–10

thymolphthalein HTh(aq) / Th–(aq) 9.4 – 10.6 colourless to blue 1.0 × 10–10

alizarin yellow R HAy(aq) / Ay–(aq) 10.1 – 12.0 yellow to red 6.9 × 10–12

indigo carmine HIc(aq) / Ic–(aq) 11.4 – 13.0 blue to yellow ~6 × 10–12

1,3,5–trinitrobenzene HNb(aq) / Nb–(aq) 12.0 – 14.0 colourless

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Colours of Common Aqueous Ions

Ionic Species

Solution Concentration

1.0 mol/L 0.010 mol/L

chromate yellow pale yellow

chromium(III) blue-green green

chromium(II) dark blue pale blue

cobalt(II) red pink

copper(I) blue-green pale blue-green

copper(II) blue pale blue

dichromate orange pale orange

iron(II) lime green colourless

iron(III) orange-yellow pale yellow

manganese(II) pale pink colourless

nickel(II) blue-green pale blue-green

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